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CaCl2 + H2CO3 = HCl + CaCO3

Input interpretation

CaCl_2 calcium chloride + H_2CO_3 carbonic acid ⟶ HCl hydrogen chloride + CaCO_3 calcium carbonate
CaCl_2 calcium chloride + H_2CO_3 carbonic acid ⟶ HCl hydrogen chloride + CaCO_3 calcium carbonate

Balanced equation

Balance the chemical equation algebraically: CaCl_2 + H_2CO_3 ⟶ HCl + CaCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CaCl_2 + c_2 H_2CO_3 ⟶ c_3 HCl + c_4 CaCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, Cl, C, H and O: Ca: | c_1 = c_4 Cl: | 2 c_1 = c_3 C: | c_2 = c_4 H: | 2 c_2 = c_3 O: | 3 c_2 = 3 c_4 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CaCl_2 + H_2CO_3 ⟶ 2 HCl + CaCO_3
Balance the chemical equation algebraically: CaCl_2 + H_2CO_3 ⟶ HCl + CaCO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 CaCl_2 + c_2 H_2CO_3 ⟶ c_3 HCl + c_4 CaCO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ca, Cl, C, H and O: Ca: | c_1 = c_4 Cl: | 2 c_1 = c_3 C: | c_2 = c_4 H: | 2 c_2 = c_3 O: | 3 c_2 = 3 c_4 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | CaCl_2 + H_2CO_3 ⟶ 2 HCl + CaCO_3

Structures

+ ⟶ +
+ ⟶ +

Names

calcium chloride + carbonic acid ⟶ hydrogen chloride + calcium carbonate
calcium chloride + carbonic acid ⟶ hydrogen chloride + calcium carbonate

Equilibrium constant

Construct the equilibrium constant, K, expression for: CaCl_2 + H_2CO_3 ⟶ HCl + CaCO_3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: CaCl_2 + H_2CO_3 ⟶ 2 HCl + CaCO_3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i CaCl_2 | 1 | -1 H_2CO_3 | 1 | -1 HCl | 2 | 2 CaCO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CaCl_2 | 1 | -1 | ([CaCl2])^(-1) H_2CO_3 | 1 | -1 | ([H2CO3])^(-1) HCl | 2 | 2 | ([HCl])^2 CaCO_3 | 1 | 1 | [CaCO3] The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([CaCl2])^(-1) ([H2CO3])^(-1) ([HCl])^2 [CaCO3] = (([HCl])^2 [CaCO3])/([CaCl2] [H2CO3])
Construct the equilibrium constant, K, expression for: CaCl_2 + H_2CO_3 ⟶ HCl + CaCO_3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: CaCl_2 + H_2CO_3 ⟶ 2 HCl + CaCO_3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i CaCl_2 | 1 | -1 H_2CO_3 | 1 | -1 HCl | 2 | 2 CaCO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression CaCl_2 | 1 | -1 | ([CaCl2])^(-1) H_2CO_3 | 1 | -1 | ([H2CO3])^(-1) HCl | 2 | 2 | ([HCl])^2 CaCO_3 | 1 | 1 | [CaCO3] The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([CaCl2])^(-1) ([H2CO3])^(-1) ([HCl])^2 [CaCO3] = (([HCl])^2 [CaCO3])/([CaCl2] [H2CO3])

Rate of reaction

Construct the rate of reaction expression for: CaCl_2 + H_2CO_3 ⟶ HCl + CaCO_3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: CaCl_2 + H_2CO_3 ⟶ 2 HCl + CaCO_3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i CaCl_2 | 1 | -1 H_2CO_3 | 1 | -1 HCl | 2 | 2 CaCO_3 | 1 | 1 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term CaCl_2 | 1 | -1 | -(Δ[CaCl2])/(Δt) H_2CO_3 | 1 | -1 | -(Δ[H2CO3])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(Δt) CaCO_3 | 1 | 1 | (Δ[CaCO3])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -(Δ[CaCl2])/(Δt) = -(Δ[H2CO3])/(Δt) = 1/2 (Δ[HCl])/(Δt) = (Δ[CaCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: CaCl_2 + H_2CO_3 ⟶ HCl + CaCO_3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: CaCl_2 + H_2CO_3 ⟶ 2 HCl + CaCO_3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i CaCl_2 | 1 | -1 H_2CO_3 | 1 | -1 HCl | 2 | 2 CaCO_3 | 1 | 1 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term CaCl_2 | 1 | -1 | -(Δ[CaCl2])/(Δt) H_2CO_3 | 1 | -1 | -(Δ[H2CO3])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(Δt) CaCO_3 | 1 | 1 | (Δ[CaCO3])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -(Δ[CaCl2])/(Δt) = -(Δ[H2CO3])/(Δt) = 1/2 (Δ[HCl])/(Δt) = (Δ[CaCO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| calcium chloride | carbonic acid | hydrogen chloride | calcium carbonate formula | CaCl_2 | H_2CO_3 | HCl | CaCO_3 Hill formula | CaCl_2 | CH_2O_3 | ClH | CCaO_3 name | calcium chloride | carbonic acid | hydrogen chloride | calcium carbonate IUPAC name | calcium dichloride | carbonic acid | hydrogen chloride | calcium carbonate
| calcium chloride | carbonic acid | hydrogen chloride | calcium carbonate formula | CaCl_2 | H_2CO_3 | HCl | CaCO_3 Hill formula | CaCl_2 | CH_2O_3 | ClH | CCaO_3 name | calcium chloride | carbonic acid | hydrogen chloride | calcium carbonate IUPAC name | calcium dichloride | carbonic acid | hydrogen chloride | calcium carbonate

Substance properties

| calcium chloride | carbonic acid | hydrogen chloride | calcium carbonate molar mass | 111 g/mol | 62.024 g/mol | 36.46 g/mol | 100.09 g/mol phase | solid (at STP) | | gas (at STP) | solid (at STP) melting point | 772 °C | | -114.17 °C | 1340 °C boiling point | | | -85 °C | density | 2.15 g/cm^3 | | 0.00149 g/cm^3 (at 25 °C) | 2.71 g/cm^3 solubility in water | soluble | | miscible | insoluble
| calcium chloride | carbonic acid | hydrogen chloride | calcium carbonate molar mass | 111 g/mol | 62.024 g/mol | 36.46 g/mol | 100.09 g/mol phase | solid (at STP) | | gas (at STP) | solid (at STP) melting point | 772 °C | | -114.17 °C | 1340 °C boiling point | | | -85 °C | density | 2.15 g/cm^3 | | 0.00149 g/cm^3 (at 25 °C) | 2.71 g/cm^3 solubility in water | soluble | | miscible | insoluble

Units

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